Multiple Choice
Which process must occur before an atom in its ground state can emit a photon?
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9. Quantum Mechanics
The Energy of Light
Multiple Choice
Which of the following frequencies of light has the highest energy?
A
1.0 \(\times\) 10^{15} \(\text{ Hz}\)
B
2.0 \(\times\) 10^{14} \(\text{ Hz}\)
C
5.0 \(\times\) 10^{14} \(\text{ Hz}\)
D
8.0 \(\times\) 10^{13} \(\text{ Hz}\)
Verified step by step guidance1
Recall the relationship between the energy of a photon and its frequency, which is given by the equation \(E = h \times f\), where \(E\) is the energy, \(h\) is Planck's constant, and \(f\) is the frequency of the light.
Understand that Planck's constant \(h\) is a fixed value (\(6.626 \times 10^{-34}\) J·s), so the energy of a photon is directly proportional to its frequency.
Compare the given frequencies: \(1.0 \times 10^{15}\) Hz, \(2.0 \times 10^{14}\) Hz, \(5.0 \times 10^{14}\) Hz, and \(8.0 \times 10^{13}\) Hz.
Since energy increases with frequency, identify the highest frequency among the options, which corresponds to the highest energy.
Conclude that the frequency \(1.0 \times 10^{15}\) Hz has the highest energy because it is the largest frequency value given.
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